Hey there!
I attached a screenshot of my chemistry notes from this year on equilibrium constants in particular. Feel free to reference this in the future if you wish.
Based on the information in my attachment, you could construct your constant like this:
![K_{eq} = \frac{[CaO][CO_{2}]}{[CaCO_{3}]}](https://tex.z-dn.net/?f=%20K_%7Beq%7D%20%3D%20%20%5Cfrac%7B%5BCaO%5D%5BCO_%7B2%7D%5D%7D%7B%5BCaCO_%7B3%7D%5D%7D%20)
I don't think it matters which order your reactants or products are in as long as you have them on the top and bottom where they need to be, so your answer will be B.
Hope this helped you out! :-)
Answer:
2800 g de ácido nítrico
Explanation:
La ecuación por la oxidación de amoniaco es:
4NH₃ + 7O₂ → 4H₂O + 2HNO₂ + 2HNO₃
Si pensamos que el oxígeno es el reactivo limitante, trabajamos con el amoniaco. Convertimos su masa a moles:
1.36 kg = 1360 g
1360 g . 1mol /17g = 80 moles
Si 4 moles de amoniaco pueden producir 2 moles de acido nítrico
80 moles producirán, (80 . 2)/4 = 40 moles.
Convertimos los moles a gramos:
40 mol . 63g /mol = 2520 g
Si le aplicamos la pureza
2520 g . 100/90 = 2800 g
Answer: The increasing wavelength of colors:
Red > Green > Blue
Explanation:
Wavelength: This is the property of wave which includes the distance between two consecutive crests or trough. This is denoted by the Greek letter Lambda and it is found by dividing the velocity of the wave with its frequency.
Wavelength of colours are
Violet: 400 - 420 nm
Indigo: 420 - 440 nm
Blue: 440 - 490 nm
Green: 490 - 570 nm
Yellow: 570 - 585 nm
Orange: 585 - 620 nm
Red: 620 - 780 nm
Answer:
The question is incomplete as some details are missing. Here is the complete question ; A chemist adds 45.0mL of a 0.434M copper(II) sulfate CuSO4 solution to a reaction flask. Calculate the mass in grams of copper(II) sulfate the chemist has added to the flask. Round your answer to 2 significant digits
Explanation:
The step by step explanation is as shown in the attachment
Answer:
The answer to your question is 1.83 x 10²⁵ particles
Explanation:
Data
particles of H₂O = ?
mass of H₂O = 546 g
Process
1.- Calculate the molar mass of Water
Molar mass = (2 x 1) + (1 x 16)
= 2 + 16
= 18 g
2.- Use proportions to find the number of particles. Use Avogadro's number.
18 g ---------------- 6.023 x 10²³ particles
546 g --------------- x
x = (546 x 6.023 x 10²³) / 18
3.- Simplification
x = 3.289 x 10²⁶ / 18
4.- Result
x = 1.83 x 10²⁵ particles
